Why do all isotopes of an element have the same chemical properties?

Question

Henry Antrim · Accepted Answer

Because each isotope of the element HAS THE SAME NUMBER OF ELECTRONS.

To a first approximation, the chemistry of an element depends on the exchange and sharing of electrons between atoms to make and break strong chemical bonds. While isotopes has different numbers of neutrons, massive, neutrally charged, nuclear particles, they have the same number of protons, massive, positively charged, nuclear particles. And the neutral atom has therefore the SAME number of electrons, as the isotopes of a given element. And if there is the same number of electrons, the chemistry of that element is essentially the same. Is this clear? Just to add that the substitution of #""^1H# by #""^2H# can introduce some change in the rate of chemical reaction. Look up the #"kinetic isotope effect..."#

Ellie Andrews · Answer

undefined Since the number of protons in an atom determines the identity of an element and how it interacts with other elements chemically, all isotopes of the same element have the same chemical properties because the number of protons in an atom determines the chemical behavior of an element. Isotopes may differ in the number of neutrons they have, which results in variations in atomic mass, but this does not affect their chemical properties.